Topic 3 & 4 - Chemical Changes and Extracting Metals and Equilibria Flashcards
(180 cards)
1
Q
- What term describes a substance that attacks metals, stonework and skin?
A
corrosive
2
Q
- Name an acidic solution found in the kitchen.
A
vinegar or fruit juice, etc.
3
Q
- Name an alkaline solution used in the kitchen.
A
bleach or oven cleaner or soap, etc.
4
Q
- What type of substance turns litmus paper red?
A
acid
5
Q
- How does an indicator show the acidity or alkalinity of solutions?
A
by changing colour
6
Q
- What pH values represent alkaline solutions?
A
above 7 or 8 to 14
7
Q
- What happens in all chemical reactions?
A
new substances are formed
8
Q
- What kind of reaction occurs between an acid and an alkali?
A
neutralisation
9
Q
- What do you call a solution that is neither acidic nor alkaline.
A
neutral
10
Q
- Give the name and formula of a common laboratory acid.
A
hydrochloric acid (HCl) or nitric acid (HNO3) or sulfuric acid (H2SO4), etc.
11
Q
- Which ion is in excess in all acidic solutions?
A
hydrogen ions or H+ ions
12
Q
- Which ion is in excess in all alkaline solutions?
A
hydroxide ions or OH– ions
13
Q
- What scale is used for measuring acidic and alkaline properties?
A
the pH scale
14
Q
- Name three examples of acid/alkali indicators apart from universal indicator.
A
litmus, methyl orange and phenolphthalein
15
Q
- What would you use to measure pH to one decimal place?
A
a pH meter
16
Q
- What pH values are acidic?
A
below 7
17
Q
- What colour is phenolphthalein in a solution with a pH of 2?
A
colourless
18
Q
- What happens to the pH as the H+ ion concentration increases?
A
it decreases
19
Q
- If a solution has the same concentration of hydrogen ions as hydroxide ions, how is it described?
A
neutral or pH = 7
20
Q
- If 2 g of salt is dissolved in 250 cm3 of solution, what is its concentration in g dm–3?
A
8 g dm–3
21
Q
- What word describes a solution that contains a large amount of solute in a small volume of solvent?
A
concentrated
22
Q
- How can a solution be made more dilute?
A
by adding solvent/water
23
Q
- If 24 g of acid is dissolved in 600 cm3 of solution, what is its concentration in g dm–3?
A
40 g dm–3
24
Q
- What happens when strong acid molecules dissolve in water?
A
they dissociate completely into ions
25
25. What kind of reaction occurs between an acid and a base?
neutralisation
26
26. What happens to the pH of an acid as it reacts with a neutraliser?
pH increases
27
27. What is formed when an acid reacts with a base like a metal oxide?
salt + water
28
28. What acid would be used to make zinc sulfate from zinc oxide?
sulfuric acid (sulphuric acid makes sulphates!)
29
29. What process can be used to separate an insoluble solid from a liquid?
filtration
30
30. How can a sample of a dissolved salt be obtained from a salt solution?
evaporation of the water
31
31. In general, what is the pH of an alkaline solution?
greater than 7
32
32. Which ions, hydrogen ions or hydroxide ions, are released by alkalis in solution?
hydroxide ions (OH-)
33
33. What colour is litmus solution in acidic solutions?
red
34
34. What name is given to substances that react with acids to form a salt and water only?
bases (bases are metal oxides and hydroxides, soluble bases are alkalis)
35
35. Which salt is formed when copper oxide reacts with sulfuric acid?
copper sulfate
36
36. What type of reaction happens between an acid and a base?
neutralisation
37
37. What type of solution has a pH of 7?
neutral
38
38. Name the acid that has the formula HCl.
hydrochloric acid
39
39. What colour is phenolphthalein in alkaline solutions?
pink (it is colourless in acid conditions)
40
40. What is the formula for sulfuric acid?
H2SO4
41
41. Name the salt produced when sodium hydroxide reacts with hydrochloric acid.
sodium chloride
42
42. Which ions, hydrogen ions or hydroxide ions, are released by acids in solution?
hydrogen ions (H+)
43
43. What substance, other than a salt, is produced when an alkali neutralises an acid?
water
44
44. What name is given to substances that are soluble bases?
alkalis
45
45. What is the formula for hydrochloric acid?
HCl
46
46. What type of solution has a pH above 7?
alkaline
47
47. What colour is phenolphthalein in acidic solutions?
colourless – not ‘clear’
48
48. Name a piece of apparatus used to measure volumes of liquid.
measuring cylinder/pipette/burette
49
49. Name the separation method used to produce crystals from a solution.
crystallisation
50
50. Name the acid needed to make ammonium nitrate.
nitric acid
51
51. Which acid can be used to make copper sulfate?
sulfuric acid
52
52. Which base can be used to make copper sulfate?
copper oxide
53
53. Which substance is needed to complete the general equation: acid + base makes salt + …?
water (BASHO)
54
54. What is the formula of nitric acid?
HNO3
55
55. What is the name of the salt formed from zinc oxide and hydrochloric acid?
zinc chloride
56
56. What is the formula of the salt formed from calcium oxide and hydrochloric acid?
CaCl2
57
57. Which ions are present in large quantities in aqueous solutions of all acids?
H+ Hydrogen ions
58
58. Which ions are present in large quantities in aqueous solutions of all alkalis?
OH– Hydroxide ions
59
59. Which gas is formed when dilute hydrochloric acid reacts with magnesium?
hydrogen (MASH)
60
60. Which gas is formed when dilute hydrochloric acid reacts with magnesium carbonate?
carbon dioxide (CASHOCO)
61
61. What acid can be used to make copper chloride?
hydrochloric acid (hydrochloric acid makes chlorides)
62
62. What gas is given off when magnesium reacts with dilute sulfuric acid?
hydrogen (MASH)
63
63. How do you identify Hydrogen gas?
gives a squeaky pop with a lighted splint
64
64. What is _seen_ when magnesium is added to dilute sulfuric acid?
effervescence/fizzing/bubbles (yes you know this is hydrogen, but you can not see that!!)
65
65. What is the formula of magnesium sulfate?
MgSO4
66
66. What gas is produced when copper carbonate is added to dilute nitric acid?
carbon dioxide (CASHOCO)
67
67. How do you test for Carbon Dioxide?
it turns limewater milky
68
68. What is the formula of the salt produced when copper carbonate reacts with nitric acid?
(Cu(NO3)2)
69
69. Sodium chloride dissolves in water to form a solution. Which is the solute?
sodium chloride
70
70. What do we call the liquid that dissolves a solute to form a solution.
solvent
71
1. What is the formula of water?
H2O
72
2. What is the formula of sodium chloride?
NaCl
73
3. What is the formula of carbon dioxide?
CO2
74
4. The formula of magnesium chloride is MgCl2. What is the ratio of magnesium ions to chloride ions?
1:2
75
5. The formula of sulfuric acid is H2SO4. How many atoms of each element are in the formula?
H = 2, S = 1, O = 4
76
6. The formula of calcium nitrate is Ca(NO3)2. How many calcium, nitrogen and oxygen atoms are in the formula?
Ca = 1, N = 2, O = 6
77
7. There are two numbers alongside chlorine in the periodic table, 17 and 35.5. What does the number 17 represent?
atomic number
78
8. What does the number 35.5 represent?
relative atomic mass
79
9. Sodium chloride has the formula NaCl. The relative atomic mass of sodium is 23 and that of chlorine is 35.5. What is the relative formula mass of NaCl?
58.5
80
10. A water molecule has the formula H2O. The relative atomic mass of hydrogen is 1 and that of oxygen is 16. What is the relative formula mass of a molecule of water?
18
81
11. What is the symbol for relative atomic mass?
Ar or RAM
82
12. What is the symbol for relative formula mass?
Mr or RFM
83
13. The relative atomic mass of hydrogen is 1. What is the relative formula mass of hydrogen molecules?
2
84
14. Sodium chloride has the formula NaCl; the relative atomic mass of sodium is 23 and that of chlorine is 35.5. What is the relative formula mass of NaCl?
58.5
85
15. A water molecule has the formula H2O; the relative atomic mass of hydrogen is 1 and that of oxygen is 16. What is the relative formula mass of water?
18
86
16. A carbon dioxide molecule has the formula CO2; the relative atomic mass of carbon is 12 and that of oxygen is 16. What is the relative formula mass of carbon dioxide?
44
87
17. What is the empirical formula of a compound with molecular formula C2H4?
CH2
88
18. What is the empirical formula of a compound with molecular formula C3H8?
C3H8
89
19. A sample of magnesium carbonate was heated in an open test tube. Why did it lose mass?
gas/carbon dioxide escaped
90
20. 100 cm3 of a solution contained 2 g of salt. What is the concentration of the salt in g dm-3?
20
91
21. A sample of copper carbonate was heated in an open test tube. Why did it lose mass?
gas/carbon dioxide escaped
92
22. Why does magnesium increase in mass when it is heated in air?
combines with oxygen
93
23. How many cm3 are there in 1 dm3?
1000
94
24. What is 250 cm3 expressed in dm3?
0.25
95
25. What is 0.5 dm3 expressed in cm3?
500
96
26. 100 cm3 of a solution contains 1.5 g of salt. What is the concentration of the salt solution in g dm3?
15
97
27. 250 cm3 of a solution contains 5 g of sugar. What is the concentration of the sugar solution in g dm3?
20
98
28. A solution of copper sulfate has concentration 10 g dm3. What mass of copper sulfate will be dissolved in 100 cm3 of solution?
1 g
99
29. 2 g of hydrogen reacts with oxygen to form 18 g of water. What mass of water will be formed from 1 g of hydrogen?
9 g
100
30. 2H2 + O2 → 2H2O. How many molecules of hydrogen are needed to react with 1 dozen molecules of oxygen to form water?
2 dozen
101
31. What is the abbreviation used for the mole, the unit for amount of substance?
mol
102
32. How many particles are there in 1 mole of particles?
6.02 x 1023
103
33. The mass of 1 mole of carbon atoms is 12 g. What is the mass of 2 moles of carbon atoms?
24 g
104
34. What is the formula for calculating the number of moles of substance from its mass in g
moles = mass (g) / RAM or RFM
105
35. Each water molecule contains three atoms. How many moles of atoms are there in 2 moles of water molecules?
6 mol
106
36. The relative formula mass of chlorine gas is 71. What is the mass of 1 mole of chlorine gas?
71 g
107
37. What is the Avogadro number?
6.02 x 1023 the number of atoms/particles in a mole
108
38. What is the emperical formula of a compound?
The simplist whole number ratio of atoms in compound
109
39. What is the law of conservation of mass?
total mass of reactants = total mass of products
110
40. How are the emperical formula and molecular formula related?
The molecular formula is a multiple of the emperical formula
111
41. What name is given to an atom that has gained or lost electrons?
ion
112
42. What type of charge is on metal and hydrogen ions?
positive
113
43. What type of charge is on most non-metal ions?
negative
114
44. What is another name for a positive ion?
cation
115
45. What is another name for a negative ion?
anion
116
46. What is the symbol for a sodium ion?
Na+
117
47. What is the symbol for a magnesium ion?
Mg2+
118
48. What is the symbol for a chloride ion?
Cl-
119
49. What is the symbol for a sulfate ion?
SO42-
120
50. In what states do ionic compounds conduct electricity?
when molten or dissolved in water
121
51. Which of these is not an electrolyte: solid sodium chloride, molten sodium chloride, aqueous sodium chloride?
solid sodium chloride
122
52. What is the name of the positively charged electrode?
anode
123
53. What type of ions are attracted to the positively charged electrode?
anions / negative ions
124
54. What is the name of the negatively charged electrode?
cathode
125
55. What type of ions are attracted to the negatively charged electrode?
cations / positive ions
126
56. H What process takes place when a substance gains electrons?
reduction
127
57. H In terms of subatomic particles, what happens to a substance when it is oxidised?
It loses electrons.
128
58. H What type of reaction takes place at the anode during electrolysis?
oxidation
129
59. What are inert electrodes made from?
graphite / platinum
130
60. What is produced at the cathode when molten lead bromide is electrolysed?
lead
131
61. What gas is formed when sodium reacts with water?
hydrogen
132
62. What solution is formed when sodium reacts with water?
sodium hydroxide
133
63. What colour is universal indicator when added to sodium hydroxide?
blue or purple
134
64. What gas is formed when magnesium is added to dilute sulfuric acid?
hydrogen (MASH)
135
65. What solution is formed when magnesium reacts with dilute sulfuric acid?
magnesium sulfate
136
66. What would you see when magnesium is added to dilute sulfuric acid?
effervescence/fizzing/bubbles/magnesium disappears
137
67. Name a metal that does not react with water or dilute acids.
copper/silver/gold/platinum
138
68. What products are formed when zinc is added to copper sulfate solution?
zinc sulfate and copper
139
69. What type of reaction takes place when zinc is added to copper sulfate solution?
displacement
140
70. Magnesium reacts with chromium nitrate solution to form magnesium nitrate and chromium. Which metal is more reactive?
magnesium
141
71. Name a metal that reacts vigorously with cold water.
potassium/sodium/rubidium/caesium/lithium/calcium
142
72. What gas is produced when a metal reacts with water?
hydrogen
143
73. How do you test for the gas produced in question 2?
It pops a lighted splint.
144
74. What type of solution is formed when a metal reacts with water - acidic, alkaline or neutral?
alkaline
145
75. What salt is formed when zinc reacts with hydrochloric acid?
zinc chloride
146
76. Complete the word equation, magnesium + copper sulfate makes ...
copper + magnesium sulfate
147
77. What type of ions are formed from metal atoms when they react with acids?
cations/positive ions
148
78. What type of reaction takes place when a substance loses oxygen?
reduction
149
79. Name a metal that occurs uncombined in the Earths crust.
gold/silver/platinum
150
80. Name a metal that could be extracted from its metal oxide by heating with carbon.
zinc/iron/copper
151
81. Name a metal that occurs uncombined in the Earths crust.
gold/silver/platinum
152
82. Name a metal, other than iron, that could be extracted from its metal oxide by heating with carbon.
zinc/copper
153
83. What compound of carbon is formed when it is heated with copper oxide?
carbon dioxide/carbon monoxide
154
84. Why is electrolysis not used to extract iron from iron oxide?
too expensive/too much energy needed
155
85. Why is aluminium not extracted by heating aluminium oxide with carbon?
aluminium is more reactive than carbon/carbon is not reactive enough to remove the oxygen
156
86. What is the aluminium oxide dissolved in to form the electrolyte for electrolysis?
molten cryolite
157
87. What are the electrodes made from?
carbon/graphite
158
88. At which electrode is the aluminium produced?
cathode/negative electrode
159
89. What type of reaction takes place when a metal is extracted from its ore?
reduction/redox
160
90. What type of reaction takes place when a metal corrodes?
oxidation/redox
161
91. What is the definition of oxidation, in terms of oxygen?
gain of oxygen
162
92. H What is the definition of oxidation, in terms of electrons?
loss of electrons
163
93. What type of reaction takes place when metals are extracted from their ores?
reduction/redox
164
94. What is the specific name for the corrosion of iron?
rusting
165
95. Which of these metals will corrode most quickly - iron, sodium, copper?
sodium
166
96. Why does sodium corrode most quickly.
most reactive metal corrodes most quickly
167
97. Which substance has been oxidised in this reaction - copper oxide + hydrogen → copper + water?
hydrogen
168
98. Which substance has been reduced in in this reaction - copper oxide + hydrogen → copper + water?
copper oxide
169
99. What name is given to a process that converts an unwanted product into a new, useful product?
recycling
170
100. Name a type of substance that can be recycled.
metal, plastic, paper, cardboard, glass, etc.
171
101. What can happen in a reversible reaction?
the products can reform the reactants
172
102. What does the term equilibrium describe?
a position of balance
173
103. What is the process used to make ammonia?
Haber Process
174
104. What is the molecular formula of ammonia?
NH3
175
105. What is the balanced symbol equation for making ammonia from Nitrogen (N2) and Hydrogen (H2)
N2 +3H2 → 2NH3
176
106. Where does nitrogen come from for use in the Haber Process?
From the fractional distillation of air
177
107. Where does Hydrogen come from for use in the Haber process?
From methane from crude oil
178
108. What conditions of pressure are required to increase the yield of ammonia in the Haber Process?
High pressure (because there are more molecules on the LHS of the equation)
179
109. The forward reaction is exothermic. What conditions of temperature are required to increase the yield of ammonia in the Haber Process?
Low temperature (The equilibrium will shit to try and produce heat)
180
110. Theoretically, a high yield of ammonia is produce at low temperature and high pressure. Why is this not used in reality?
Low temperatue will result in a slow rate of reaction. High pressures are expensive and dangerous.
